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Eileen Si 1G
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Joined: Fri Aug 30, 2019 12:17 am


Postby Eileen Si 1G » Sun Nov 10, 2019 3:35 am

How do dipole moments determine polarity, like whether a covalent bond is polar or nonpolar?

Amanda Lin 2I
Posts: 101
Joined: Sat Aug 17, 2019 12:15 am

Re: Polarity

Postby Amanda Lin 2I » Sun Nov 10, 2019 4:51 am

A molecule with a dipole moment is polar. A molecule with no dipole moment is nonpolar.

Rebecca Epner 4A
Posts: 53
Joined: Sat Aug 17, 2019 12:18 am

Re: Polarity

Postby Rebecca Epner 4A » Sun Nov 10, 2019 11:40 am

If a molecule is made up of two other same atoms, the molecule is nonpolar because the electronegativities are the same. Also, be sure to note that the bonds within a molecule may be polar even though the overall molecule is nonpolar.

Frederick Keith_4C
Posts: 65
Joined: Thu Sep 26, 2019 12:19 am

Re: Polarity

Postby Frederick Keith_4C » Sun Nov 10, 2019 12:09 pm

A dipole moment is the mathematical product of the separation of the ends of a dipole and the magnitude of the charges.
So a polar molecule will have a dipole moment with an arrow pointed towards the more electronegative atom. And a nonpolar molecule won't have a dipole moment.
Polar molecules must contain polar bonds due to a difference in electronegatvity between the bonded atoms.
Electronegativity is the tendency of an atom to attract a shared pair of electrons towards itself

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